The document describes changes made by the Cambridge International Examinations (CIE) to question papers for popular assessments with large candidature. CIE now uses two similar but distinct variants for some question papers instead of just one. The content and standard assessed remains the same between variants. Centres will receive both variants, allowing access to more past exam material. The relationship between question papers, mark schemes, and examiner reports is shown in a table. Any questions about these changes should be directed to CIE Customer Services. The titles of the variant items should clearly indicate which variant they correspond to.

1. w
w
ap
eP
m
e
tr
.X
w
om
.c
s
er
Location Entry Codes
As part of CIE’s continual commitment to maintaining best practice in assessment, CIE uses
different variants of some question papers for our most popular assessments with large and
widespread candidature. The question papers are closely related and the relationships between
them have been thoroughly established using our assessment expertise. All versions of the
paper give assessment of equal standard.
The content assessed by the examination papers and the type of questions is unchanged.
This change means that for this component there are now two variant Question Papers, Mark
Schemes and Principal Examiner’s Reports where previously there was only one. For any
individual country, it is intended that only one variant is used. This document contains both
variants which will give all Centres access to even more past examination material than is usually
the case.
The diagram shows the relationship between the Question Papers, Mark Schemes and Principal
Examiners’ Reports that are available.
Question Paper
Mark Scheme
Principal Examiner’s
Report
Introduction
Introduction
Introduction
First variant Question Paper
First variant Mark Scheme
First variant Principal
Examiner’s Report
Second variant Question
Paper
Second variant Mark
Scheme
Second variant Principal
Examiner’s Report
Who can I contact for further information on these changes?
Please direct any questions about this to CIE’s Customer Services team at:
international@cie.org.uk
The titles for the variant items should correspond with the table above, so that at the top of the
first page of the relevant part of the document and on the header, it has the words:
•
First variant Question Paper / Mark Scheme / Principal Examiner’s Report
•
Second variant Question Paper / Mark Scheme / Principal Examiner’s Report
or
as appropriate.

2. First Variant Question Paper
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS
International General Certificate of Secondary Education
*5310297965*
0620/31
CHEMISTRY
May/June 2009
Paper 3 (Extended)
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use a pencil for any diagrams, graphs or rough working.
Do not use staples, paper clips, highlighters, glue or correction fluid.
For Examiner's Use
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
A copy of the Periodic Table is printed on page 16.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part
questions.
1
2
3
4
5
6
7
8
9
Total
This document consists of 15 printed pages and 1 blank pages.
IB09 06_0620_31/5RP
© UCLES 2009
[Turn over

3. 2
1
Some grass is crushed and mixed with the solvent, propanone. The colour pigments are
extracted to give a deep green solution.
(a) (i) Draw a labelled diagram to describe how you could show that there is more than
one coloured pigment in the green solution.
[3]
(ii) Given a pure sample of chlorophyll, how could you show that the green solution
from the grass contained chlorophyll?
[2]
(b) Explain the role of chlorophyll in green plants.
[3]
[Total: 8]
© UCLES 2009
0620/31/M/J/09
For
Examiner's
Use

4. 3
2
The results of experiments on electrolysis using inert electrodes are given in the table.
For
Examiner's
Use
Complete the table; the first line has been completed as an example.
electrolyte
molten lead(II)
bromide
change at negative
electrode
change at positive
electrode
change to
electrolyte
lead formed
bromine formed
used up
potassium formed
iodine formed
used up
hydrogen formed
bromine formed
potassium hydroxide
formed
dilute aqueous
sodium chloride
aqueous copper(II)
sulfate
[Total: 8]
© UCLES 2009
0620/31/M/J/09
[Turn over

5. 4
3
The following is a list of the electron distributions of atoms of unknown elements.
element
For
Examiner's
Use
electron distribution
A
2,5
B
2,8,4
C
2,8,8,2
D
2,8,18,8
E
2,8,18,8,1
F
2,8,18,18,7
(a) Choose an element from the list for each of the following descriptions.
(i) It is a noble gas.
(ii) It is a soft metal with a low density.
(iii) It can form a covalent compound with element A.
(iv) It has a giant covalent structure similar to diamond.
(v) It can form a negative ion of the type X3-.
[5]
(b) Elements C and F can form an ionic compound.
(i) Draw a diagram that shows the formula of this compound, the charges on the ions
and the arrangement of the valency electrons around the negative ion.
Use o to represent an electron from an atom of C.
Use x to represent an electron from an atom of F.
[3]
(ii) Predict two properties of this compound.
[2]
[Total: 10]
© UCLES 2009
0620/31/M/J/09

6. 5
4
The reactivity series of metals given below contains both familiar and unfamiliar elements.
For most of the unfamiliar elements, which are marked *, their common oxidation states are
given.
* barium
Ba
* lanthanum
La
For
Examiner's
Use
(+3)
magnesium
zinc
* chromium
Cr (+2), (+3), (+6)
iron
copper
* palladium
(+2)
Choose metal(s) from the above list to answer the following questions.
(i) Which two metals would not react with dilute hydrochloric acid?
[2]
(ii) Which two unfamiliar metals (*) would react with cold water?
[2]
(iii) What is the oxidation state of barium?
[1]
(iv) Name an unfamiliar metal (*) whose oxide cannot be reduced by carbon.
[1]
(v) Why should you be able to predict that metals such as iron and chromium have
more than one oxidation state?
[1]
[Total: 7]
© UCLES 2009
0620/31/M/J/09
[Turn over

7. 6
5
For
Examiner's
Use
Insoluble salts are made by precipitation.
(a) A preparation of the insoluble salt calcium fluoride is described below.
To 15 cm3 of aqueous calcium chloride, 30 cm3 of aqueous sodium fluoride is added.
The concentration of both solutions is 1.00 mol / dm3. The mixture is filtered and the
precipitate washed with distilled water. Finally, the precipitate is heated in an oven.
(i) Complete the equation.
Ca2+ + ...…….F-
………......
[2]
(ii) Why is the volume of sodium fluoride solution double that of the calcium chloride
solution?
[1]
(iii) Why is the mixture washed with distilled water?
[1]
(iv) Why is the solid heated?
[1]
© UCLES 2009
0620/31/M/J/09

8. 7
(b) The formulae of insoluble compounds can be found by precipitation reactions.
To 12.0 cm3 of an aqueous solution of the nitrate of metal T was added 2.0 cm3 of
aqueous sodium phosphate, Na3PO4. The concentration of both solutions was
1.00 mol / dm3. When the precipitate had settled, its height was measured.
For
Examiner's
Use
solution
precipitate of
the phosphate
of metal T
height of
precipitate
The experiment was repeated using different volumes of the phosphate solution. The
results are shown on the following graph.
16
12
height of
precipitate
/ mm
8
4
0
0
2
4
6
8
10
volume of phosphate solution / cm
12
14
3
What is the formula of the phosphate of metal T? Give your reasoning.
[3]
[Total: 8]
© UCLES 2009
0620/31/M/J/09
[Turn over

9. 8
6
Ammonia is manufactured by the Haber process.
N2(g) +
3H2(g)
2NH3(g)
For
Examiner's
Use
the forward reaction is exothermic
(a) (i) Name the raw materials from which nitrogen and hydrogen are obtained.
nitrogen from
[1]
hydrogen from
[1]
(ii) Name the catalyst used in this process.
[1]
(iii) What is the most important use of ammonia?
[1]
(b) The following graph shows how the percentage of ammonia in the equilibrium mixture
changes with temperature.
% ammonia
at equilibrium
0
0
temperature
(i) Explain the term equilibrium.
[2]
(ii) How does the percentage of ammonia vary with temperature?
[1]
© UCLES 2009
0620/31/M/J/09

10. 9
(c) (i) Sketch a graph which shows how the percentage of ammonia in the equilibrium
mixture varies with pressure.
For
Examiner's
Use
% ammonia
at equilibrium
0
0
pressure
[1]
(ii) Explain why the graph has the shape shown.
[2]
[Total: 10]
© UCLES 2009
0620/31/M/J/09
[Turn over

11. 10
7
Hydrogen reacts with the halogens to form hydrogen halides.
(a) Bond energy is the amount of energy, in kJ, that must be supplied (endothermic) to
break one mole of a bond.
bond
bond energy in kJ / mol
H─H
+436
Cl─Cl
+242
H─Cl
+431
Use the above data to show that the following reaction is exothermic.
H─H
+
Cl─Cl
2H─Cl
[3]
© UCLES 2009
0620/31/M/J/09
For
Examiner's
Use

12. 11
(b) They react with water to form acidic solutions.
HCl
+
H2O
H3O+
+
Cl -
HF
+
H2O
H3O+
+
For
Examiner's
Use
F-
(i) Explain why water behaves as a base in both of these reactions.
[2]
(ii) At equilibrium, only 1% of the hydrogen chloride exists as molecules, the rest has
formed ions. In the other equilibrium, 97% of the hydrogen fluoride exists as
molecules, only 3% has formed ions.
What does this tell you about the strength of each acid?
[2]
(iii) How would the pH of these two solutions differ?
[1]
[Total: 8]
© UCLES 2009
0620/31/M/J/09
[Turn over

13. 12
8
Lactic acid can be made from corn starch.
CH3
CH
For
Examiner's
Use
COOH
OH
lactic acid
It polymerises to form the polymer, polylactic acid (PLA ) which is biodegradable.
(a) Suggest two advantages that PLA has compared with a polymer made from petroleum.
[2]
(b) The structure of PLA is given below.
CH3
O
O
CH
C
CH3
O
CH
(i) What type of compound contains the group that is circled?
[1]
(ii) Complete the following sentence.
Lactic acid molecules can form this group because they contain both an
group and an
group.
[2]
(iii) Is the formation of PLA, an addition or condensation polymerisation? Give a
reason for your choice.
[2]
© UCLES 2009
0620/31/M/J/09

14. 13
(c) When lactic acid is heated, acrylic acid is formed.
H
C
C
H
H
H
OH
H
lactic acid
H
C
COOH
For
Examiner's
Use
H
C
COOH
acrylic acid
(i) Complete the word equation for the action of heat on lactic acid.
lactic acid →
+
[1]
(ii) Describe a test that would distinguish between lactic acid and acrylic acid.
test
result for lactic acid
result for acrylic acid
[3]
(iii) Describe a test, other than using an indicator, which would show that both
chemicals contain an acid group.
test
result
[2]
[Total: 13]
© UCLES 2009
0620/31/M/J/09
[Turn over

15. 14
9
Quantities of chemicals, expressed in moles, can be used to find the formula of a
compound, to establish an equation and to determine reacting masses.
(a) A compound contains 72% magnesium and 28% nitrogen. What is its empirical
formula?
[2]
(b) A compound contains only aluminium and carbon. 0.03 moles of this compound reacted
with excess water to form 0.12 moles of Al(OH)3 and 0.09 moles of CH4.
Write a balanced equation for this reaction.
[2]
(c) 0.07 moles of silicon reacts with 25 g of bromine.
Si
+
2Br2
SiBr4
(i) Which one is the limiting reagent? Explain your choice.
[3]
(ii) How many moles of SiBr4 are formed?
[1]
[Total: 8]
© UCLES 2009
0620/31/M/J/09
For
Examiner's
Use

16. 15
BLANK PAGE
0620/31/M/J/09

17. © UCLES 2009
24
40
Sodium
Calcium
88
0620/31/M/J/09
89
Key
b
X
a
b = proton (atomic) number
X = atomic symbol
a = relative atomic mass
*58-71 Lanthanoid series
90-103 Actinoid series
88
Ac
Actinium
Ra
Radium
Fr
Francium
87
*
Hafnium
72
Lanthanum
57
Hf
La
40
Zirconium
Zr
91
Titanium
178
Yttrium
22
48
Ti
139
39
Y
89
Scandium
21
227
Barium
Caesium
56
Cs
45
Sc
226
55
137
Ba
133
Strontium
Rubidium
38
Rb
37
Sr
85
20
Potassium
19
Ca
39
Magnesium
Na
12
Mg
23
Beryllium
4
Lithium
K
11
3
9
Be
7
II
Li
I
93
Ta
181
Niobium
Nb
90
58
73
52
96
Mo
W
184
141
Pa
Thorium
55
Tc
186
Re
144
Nd
92
60
Uranium
U
238
Neodymium
75
Rhenium
43
Technetium
25
Manganese
Mn
29
30
65
8
9
VII
2
0
Ru
101
Iron
190
Pm
Osmium
Os
Np
93
Neptunium
61
Promethium
76
44
Ruthenium
26
56
Fe
Sm
150
Iridium
Pu
94
Plutonium
62
Eu
152
Platinum
Am
95
Americium
63
Europium
78
195
Pt
Ir
46
Palladium
Pd
106
Nickel
Ni
192
Samarium
77
45
Rhodium
Rh
103
Cobalt
Co
Gd
157
Gold
Au
197
Silver
96
64
Curium
Cm
Gadolinium
79
47
Ag
108
Copper
Cu
201
Bk
Terbium
Tb
159
Mercury
Hg
97
Berkelium
65
80
48
Cadmium
Cd
112
Zinc
Zn
11
70
Dy
162
Thallium
Tl
204
Indium
Cf
98
Californium
66
Es
Holmium
Ho
165
Lead
Pb
207
Tin
99
Einsteinium
67
82
50
119
Sn
In
32
Germanium
Ge
73
Silicon
115
Gallium
Ga
Dysprosium
81
49
31
13
Aluminium
Si
Al
14
28
Carbon
27
Boron
12
C
14
75
Sb
122
Arsenic
As
Bi
209
Fermium
Fm
Erbium
Er
167
Bismuth
100
68
83
51
Antimony
33
15
Phosphorus
P
31
Nitrogen
N
Se
79
Sulfur
S
32
Oxygen
Po
169
Md
Thulium
Tm
101
Mendelevium
69
84
Polonium
52
Tellurium
Te
128
Selenium
34
16
16
O
Yb
173
Astatine
At
Iodine
I
127
Bromine
Br
80
Chlorine
No
102
Nobelium
70
Ytterbium
85
53
35
17
Cl
35.5
Fluorine
F
19
Lr
Lutetium
Lu
175
Radon
Rn
Xenon
Xe
131
Krypton
Kr
84
Argon
Ar
40
Neon
103
Lawrencium
71
86
54
36
18
10
Ne
20
Helium
Hydrogen
B
4
28
64
7
VI
He
27
59
6
V
H
59
5
IV
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
91
Protactinium
Th
232
Praseodymium
Cerium
59
Pr
Ce
74
Tungsten
42
Molybdenum
24
Chromium
Cr
140
Tantalum
41
23
Vanadium
V
51
1
III
1
Group
DATA SHEET
The Periodic Table of the Elements
16
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of
Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.

18. Second Variant Question Paper
UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS
International General Certificate of Secondary Education
*0583100121*
0620/32
CHEMISTRY
May/June 2009
Paper 3 (Extended)
1 hour 15 minutes
Candidates answer on the Question Paper.
No Additional Materials are required.
READ THESE INSTRUCTIONS FIRST
Write your Centre number, candidate number and name on all the work you hand in.
Write in dark blue or black pen.
You may use a pencil for any diagrams, graphs or rough working.
Do not use staples, paper clips, highlighters, glue or correction fluid.
For Examiner's Use
DO NOT WRITE IN ANY BARCODES.
Answer all questions.
A copy of the Periodic Table is printed on page 16.
At the end of the examination, fasten all your work securely together.
The number of marks is given in brackets [ ] at the end of each question or part
questions.
1
2
3
4
5
6
7
8
9
Total
This document consists of 15 printed pages and 1 blank page.
IB09 06_0620_32/4RP
© UCLES 2009
[Turn over

19. 2
1
Some grass is crushed and mixed with the solvent, propanone. The colour pigments are
extracted to give a deep green solution.
(a) (i) Draw a labelled diagram to describe how you could show that there is more than
one coloured pigment in the green solution.
[3]
(ii) Given a pure sample of chlorophyll, how could you show that the green solution
from the grass contained chlorophyll?
[2]
(b) Explain the role of chlorophyll in green plants.
[3]
[Total: 8]
© UCLES 2009
0620/32/M/J/09
For
Examiner's
Use

20. 3
2
The results of experiments on electrolysis using inert electrodes are given in the table.
For
Examiner's
Use
Complete the table; the first line has been completed as an example.
electrolyte
change at negative
electrode
change at positive
electrode
change to electrolyte
lead formed
bromine formed
used up
lithium formed
chlorine formed
used up
hydrogen formed
molten lead(II)
bromide
bromine formed
potassium hydroxide
formed
dilute aqueous sodium
chloride
aqueous copper(II)
sulfate
[Total: 8]
© UCLES 2009
0620/32/M/J/09
[Turn over

21. 4
3
The following is a list of the electron distributions of atoms of unknown elements.
element
For
Examiner's
Use
electron distribution
A
2,6
B
2,8,4
C
2,8,8,2
D
2,8,18,8
E
2,8,18,8,1
F
2,8,18,18,7
(a) Choose an element from the list for each of the following descriptions.
(i) It is a noble gas.
(ii) It is a soft metal with a low density.
(iii) It can form a covalent compound with element A.
(iv) It has a giant covalent structure similar to diamond.
(v) It is a diatomic gas with molecules of the type X2.
[5]
(b) Elements C and A can form an ionic compound.
(i) Draw a diagram that shows the formula of this compound, the charges on the ions
and the arrangement of the valency electrons around the negative ion.
Use o to represent an electron from an atom of C.
Use x to represent an electron from an atom of A.
[3]
(ii) Predict two properties of this compound.
[2]
[Total: 10]
© UCLES 2009
0620/32/M/J/09

22. 5
4
The reactivity series of metals given below contains both familiar and unfamiliar elements.
For most of the unfamiliar elements, which are marked *, their common oxidation states are
given.
* barium
Ba
* lanthanum
La
For
Examiner's
Use
(+3)
magnesium
zinc
* chromium
Cr (+2), (+3), (+6)
iron
copper
* palladium
(+2)
Choose metal(s) from the above list to answer the following questions.
(i) Which two metals would not react with dilute hydrochloric acid?
[2]
(ii) Which two unfamiliar metals (*) would react with cold water?
[2]
(iii) What is the oxidation state of barium?
[1]
(iv) Name an unfamiliar metal (*) whose oxide cannot be reduced by carbon.
[1]
(v) Why should you be able to predict that metals such as iron and chromium have
more than one oxidation state?
[1]
[Total: 7]
© UCLES 2009
0620/32/M/J/09
[Turn over

23. 6
5
Insoluble salts are made by precipitation.
For
Examiner's
Use
(a) A preparation of the insoluble salt iron fluoride is described below.
To 15 cm3 of aqueous iron(III) chloride, 45 cm3 of aqueous sodium fluoride is added.
The concentration of both solutions is 1.00 mol / dm3. The mixture is filtered and the
precipitate washed with distilled water. Finally, the precipitate is heated in an oven.
(i) Complete the equation.
Fe3+ + ...…….F-
………......
[2]
(ii) Why is the volume of sodium fluoride solution three times that of the iron(III)
chloride solution?
[1]
(iii) Why is the mixture washed with distilled water?
[1]
(iv) Why is the solid heated?
[1]
© UCLES 2009
0620/32/M/J/09

24. 7
(b) The formulae of insoluble compounds can be found by precipitation reactions.
To 18.0 cm3 of an aqueous solution of the nitrate of metal T was added 2.0 cm3 of
aqueous sodium phosphate, Na3PO4. The concentration of both solutions was
1.00 mol / dm3. When the precipitate had settled, its height was measured.
For
Examiner's
Use
solution
precipitate of
the phosphate
of metal T
height of
precipitate
The experiment was repeated using different volumes of the phosphate solution. The
results are shown on the following graph.
16
12
height of
precipitate
/ mm
8
4
0
0
2
4
6
8
10
volume of phosphate solution / cm
12
14
3
What is the formula of the phosphate of metal T? Give your reasoning.
[3]
[Total: 8]
© UCLES 2009
0620/32/M/J/09
[Turn over

25. 8
6
Ammonia is manufactured by the Haber process.
N2(g) +
3H2(g)
2NH3(g)
For
Examiner's
Use
the forward reaction is exothermic
(a) (i) Name the raw materials from which nitrogen and hydrogen are obtained.
nitrogen from
[1]
hydrogen from
[1]
(ii) Name the catalyst used in this process.
[1]
(iii) What is the most important use of ammonia?
[1]
(b) The following graph shows how the percentage of ammonia in the equilibrium mixture
changes with pressure.
% ammonia
at equilibrium
0
0
pressure
(i) Explain the term equilibrium.
[2]
(ii) How does the percentage of ammonia vary with pressure?
[1]
© UCLES 2009
0620/32/M/J/09

26. 9
(c) (i) Sketch a graph which shows how the percentage of ammonia in the equilibrium
mixture varies with temperature.
For
Examiner's
Use
% ammonia
at equilibrium
0
0
temperature
[1]
(ii) Explain why the graph has the shape shown.
[2]
[Total: 10]
© UCLES 2009
0620/32/M/J/09
[Turn over

27. 10
7
Hydrogen reacts with the halogens to form hydrogen halides.
(a) Bond energy is the amount of energy, in kJ, that must be supplied (endothermic) to
break one mole of a bond.
bond
bond energy in kJ / mol
H─H
+436
F─F
+158
H─F
+562
Use the above data to show that the following reaction is exothermic.
H─H
+
F─F
2H─F
[3]
© UCLES 2009
0620/32/M/J/09
For
Examiner's
Use

28. 11
(b) They react with water to form acidic solutions.
HCl
+
H2O
H3O+
+
Cl -
HF
+
H2O
H3O+
+
For
Examiner's
Use
F-
(i) Explain why water behaves as a base in both of these reactions.
[2]
(ii) At equilibrium, only 1% of the hydrogen chloride exists as molecules, the rest has
formed ions. In the other equilibrium, 97% of the hydrogen fluoride exists as
molecules, only 3% has formed ions.
What does this tell you about the strength of each acid?
[2]
(iii) How would the pH of these two solutions differ?
[1]
[Total: 8]
© UCLES 2009
0620/32/M/J/09
[Turn over

29. 12
8
Lactic acid can be made from corn starch.
CH3
CH
For
Examiner's
Use
COOH
OH
lactic acid
It polymerises to form the polymer, polylactic acid (PLA ) which is biodegradable.
(a) Suggest two advantages that PLA has compared with a polymer made from petroleum.
[2]
(b) The structure of PLA is given below.
CH3
O
O
CH
C
CH3
O
CH
(i) What type of compound contains the group that is circled?
[1]
(ii) Complete the following sentence.
Lactic acid molecules can form this group because they contain both an
group and an
group.
[2]
(iii) Is the formation of PLA, an addition or condensation polymerisation? Give a
reason for your choice.
[2]
© UCLES 2009
0620/32/M/J/09

30. 13
(c) When lactic acid is heated, acrylic acid is formed.
H
C
C
H
H
H
OH
H
lactic acid
H
C
COOH
For
Examiner's
Use
H
C
COOH
acrylic acid
(i) Complete the word equation for the action of heat on lactic acid.
lactic acid →
+
[1]
(ii) Describe a test that would distinguish between lactic acid and acrylic acid.
test
result for lactic acid
result for acrylic acid
[3]
(iii) Describe a test, other than using an indicator, which would show that both
chemicals contain an acid group.
test
result
[2]
[Total: 13]
© UCLES 2009
0620/32/M/J/09
[Turn over

31. 14
9
Quantities of chemicals, expressed in moles, can be used to find the formula of a
compound, to establish an equation and to determine reacting masses.
(a) A compound contains 72% magnesium and 28% nitrogen. What is its empirical
formula?
[2]
(b) A compound contains only aluminium and carbon. 0.03 moles of this compound reacted
with excess water to form 0.12 moles of Al(OH)3 and 0.09 moles of CH4.
Write a balanced equation for this reaction.
[2]
(c) 0.08 moles of silicon reacts with 7.2 g of fluorine.
Si
+
2F2
SiF4
(i) Which one is the limiting reagent? Explain your choice.
[3]
(ii) How many moles of SiF4 are formed?
[1]
[Total: 8]
© UCLES 2009
0620/32/M/J/09
For
Examiner's
Use

32. 15
BLANK PAGE
0620/32/M/J/09

33. © UCLES 2009
24
40
Sodium
Calcium
88
0620/32/M/J/09
89
Key
b
X
a
b = proton (atomic) number
X = atomic symbol
a = relative atomic mass
*58-71 Lanthanoid series
90-103 Actinoid series
88
Ac
Actinium
Ra
Radium
Fr
Francium
87
*
Hafnium
72
Lanthanum
57
Hf
La
40
Zirconium
Zr
91
Titanium
178
Yttrium
22
48
Ti
139
39
Y
89
Scandium
21
227
Barium
Caesium
56
Cs
45
Sc
226
55
137
Ba
133
Strontium
Rubidium
38
Rb
37
Sr
85
20
Potassium
19
Ca
39
Magnesium
Na
12
Mg
23
Beryllium
4
Lithium
K
11
3
9
Be
7
II
Li
I
93
Ta
181
Niobium
Nb
90
58
73
52
96
Mo
W
184
141
Pa
Thorium
55
Tc
186
Re
144
Nd
92
60
Uranium
U
238
Neodymium
75
Rhenium
43
Technetium
25
Manganese
Mn
29
30
65
8
9
VII
2
0
Ru
101
Iron
190
Pm
Osmium
Os
Np
93
Neptunium
61
Promethium
76
44
Ruthenium
26
56
Fe
Sm
150
Iridium
Ir
192
Pu
94
Plutonium
62
Samarium
77
45
Rhodium
Rh
103
Cobalt
Co
195
Eu
152
Platinum
Pt
Am
95
Americium
63
Europium
78
46
Palladium
Pd
106
Nickel
Ni
Gd
157
Gold
Au
197
Silver
96
64
Curium
Cm
Gadolinium
79
47
Ag
108
Copper
Cu
201
Bk
Terbium
Tb
159
Mercury
Hg
97
Berkelium
65
80
48
Cadmium
Cd
112
Zinc
Zn
11
70
Dy
162
Thallium
Tl
204
Indium
In
115
Gallium
Ga
Cf
98
Californium
66
Dysprosium
81
49
31
13
Aluminium
119
Es
Holmium
Ho
165
Lead
Pb
207
Tin
Sn
99
Einsteinium
67
82
50
32
Germanium
Ge
73
Silicon
Si
Al
14
28
Carbon
27
Boron
12
C
14
75
Sb
122
Arsenic
As
Bi
209
Fermium
Fm
Erbium
Er
167
Bismuth
100
68
83
51
Antimony
33
15
Phosphorus
P
31
Nitrogen
N
Se
79
Sulfur
S
32
Oxygen
Po
169
Md
Thulium
Tm
101
Mendelevium
69
84
Polonium
52
Tellurium
Te
128
Selenium
34
16
16
O
Yb
173
Astatine
At
Iodine
I
127
Bromine
Br
80
Chlorine
No
102
Nobelium
70
Ytterbium
85
53
35
17
Cl
35.5
Fluorine
F
19
Lr
Lutetium
Lu
175
Radon
Rn
Xenon
Xe
131
Krypton
Kr
84
Argon
Ar
40
Neon
103
Lawrencium
71
86
54
36
18
10
Ne
20
Helium
Hydrogen
B
4
28
64
7
VI
He
27
59
6
V
H
59
5
IV
The volume of one mole of any gas is 24 dm3 at room temperature and pressure (r.t.p.).
91
Protactinium
Th
232
Praseodymium
Cerium
59
Pr
Ce
74
Tungsten
42
Molybdenum
24
Chromium
Cr
140
Tantalum
41
23
Vanadium
V
51
1
III
1
Group
DATA SHEET
The Periodic Table of the Elements
16
Permission to reproduce items where third-party owned material protected by copyright is included has been sought and cleared where possible. Every
reasonable effort has been made by the publisher (UCLES) to trace copyright holders, but if any items requiring clearance have unwittingly been included, the
publisher will be pleased to make amends at the earliest possible opportunity.
University of Cambridge International Examinations is part of the Cambridge Assessment Group. Cambridge Assessment is the brand name of University of
Cambridge Local Examinations Syndicate (UCLES), which is itself a department of the University of Cambridge.